The molecular geometry of the Krypton Pentachloride Cation (KrCl₅⁺) can be determined by analyzing the valence electrons and the arrangement of surrounding atoms. Krypton, being a noble gas in Group 8A, typically has 8 valence electrons. However, in this cation, it loses one electron, resulting in 7 valence electrons. Each chlorine atom, from Group 7A, contributes 7 valence electrons as well.

When constructing the Lewis structure, Krypton forms single bonds with five chlorine atoms, utilizing 5 of its 7 valence electrons. This leaves 2 electrons, which are represented as a lone pair on the Krypton atom. The presence of five bonding pairs (from the chlorine atoms) and one lone pair leads to a specific arrangement of these electron groups.

In this scenario, the molecular geometry is classified as square pyramidal. This geometry arises because the five chlorine atoms occupy the corners of a square base, while the lone pair occupies an axial position above the center of the square. The square pyramidal shape is characterized by its unique arrangement, which influences the molecule's properties and reactivity.